How to Calculate the Mass of Water Needed to Produce Oxygen Gas?
What mass of H2O, in grams, must react to produce 50.00 g of O2?
a) 14.07
b) 23.05
c) 28.14
d) 56.28
56.28 g of H2O is needed
The balanced chemical reaction is: 2H2O = 2H2 + O2. We are given the amount of oxygen to be produced in the reaction, which is 50.00 g. By using the molar masses of O2 and H2O, we can calculate the mass of H2O needed.
To calculate the mass of H2O needed, we can use the following formula:
50 g (1 mol O2 / 32 g O2) * (2 mol H2O / 1 mol O2) * (18.01 g H2O / 1 mol H2O) = 56.28 g of H2O
Therefore, the correct answer is the last option, 56.28 g of H2O is needed to react and produce 50.00 g of O2.
Molar Mass:The molar mass of a substance is the mass in grams of one mole of that substance. In this case, the molar mass of a compound is determined by adding up the atomic masses of each element in the compound. For example, the molar mass of H2O is 18.01 g/mol, and the molar mass of O2 is 32.00 g/mol.
Therefore, the molar mass plays a crucial role in determining the amount of reactants needed when performing chemical reactions.